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Use the data on the next slide for the reaction of
hypochlorite ion with iodide ion...
11.4 The hypochlorite ion oxidizes the iodide ion in aqueous solution as represented by the equation,...
11.4 The hypochlorite ion oxidizes the iodide ion in aqueous solution as represented by the equation, oci" + Iº +01+ Cl". The rate of formation of or is given by the rate law Rate = k (1"[oci") (OH) The overall reaction order is a. o b. 1 o 2 d. 3 e. 4
The iodide ion reacts with hypochlorite ion (the active ingredient in chlorine bleaches) in the following...
The iodide ion reacts with hypochlorite ion (the active ingredient in chlorine bleaches) in the following way: OCl?+I??OI?+Cl?. This rapid reaction gives the following rate data: [OCl?](M) [I]?(M) Rate (M/s) 1.5×10?3 1.5×10?3 1.36×10?4 3.0×10?3 1.5×10?3 2.72×10?4 1.5×10?3 3.0×10?3 2.72×10?4 Write the rate law for this reaction. Calculate the rate constant with proper units. Calculate the rate when [OCl?]= 1.8×10?3 M and [I?]= 6.0×10?4 M .
The iodide ion reacts with hypochlorite ion (the active ingredient in chlorine bleaches) in the following...
The iodide ion reacts with hypochlorite ion (the active ingredient in chlorine bleaches) in the following way: OCl−+I−→OI−+Cl− This rapid reaction gives the following rate data: [OCl−] (M) [I−] (M) Initial Rate (M/s) 1.5×10−3 1.5×10−3 1.36×10−4 3.0×10−3 1.5×10−3 2.72×10−4 1.5×10−3 3.0×10−3 2.72×10−4 Calculate the rate constant with proper units. Express the rate constant to two significant figures. Indicate the multiplication of units, as necessary, explicitly either with a multiplication dot or a dash (e.g. ft * lb or ft- lb)....
1. The hydroxide ion (OH-) catalyzes the reaction below, and rate data was obtained: OCI +...
1. The hydroxide ion (OH-) catalyzes the reaction below, and rate data was obtained: OCI + ----> OI + Cl Experiment # [OCI]. (M) [1]. (M) [OH-]. Initial Rate (M/s) (M) 0.0040 0.0020 1.00 0.00184 2 0.0020 0.0040 1.00 0.00092 0.0020 0.0020 1.00 0.00046 0.0020 0.50 0.00046 0.0020 0.0020 0.25 0.00046 0.0020 Determine the rate law expression for this reaction (10 pts) What is the value of k (with proper units)? (5 pts)
The peroxydisulfate ion (S2O82-) reacts with the iodide ion in aqueous solution via the reaction: S2O82-...
The peroxydisulfate ion (S2O82-) reacts with the iodide ion in aqueous solution via the reaction: S2O82- (aq) + 3I- → 2SO42- + I3- (aq) An aqueous solution containing 0.050 M of S2O82-ion and 0.072 M of I-is prepared, and the progress of the reaction followed by measuring [I-].The data obtained is given the table below. Time (s) 0.000 400.0 800.0 1200.0 1600.0 [I-] (M) 0.072 0.057 0.046 0.037 0.029 The concentration of S2O82- remaining at 800 s is ________ M....
Questions 1-5 For #1 - #5 questions of Exp. 16, complete the following chemical reaction equations...
Questions 1-5
For #1 - #5 questions of Exp. 16, complete the following chemical reaction equations (1 point each). For example, Ag+ (aq) + Cl - (aq) + AgCl (s, I white) 1. For another example, silver precipitation, AgCl (s), reacts with 15 M ammonia aqueous solution. Complete this chemical reaction equation. AgCl (s) + 2NH3 (aq) → Ag(NH3)2 + (aq) + Cl(aq) 2. The silver complex ion, one of the products from above chemical reaction equation, reacts with 6...
Consider the reaction of peroxydisulfate ion (S20;-) with iodide ion (I) in aqueous solution: S2O3- (aq)...
Consider the reaction of peroxydisulfate ion (S20;-) with iodide ion (I) in aqueous solution: S2O3- (aq) + 31- (aq) +250- (aq) +15 (aq). At a particular temperature the rate of disappearance of S20% varies with reactant concentrations in the following manner: 1 Experiment S20%- (M) I- (M) Initial Rate (M/s) 0.018 0.036 2.6 x 10-6 0.027 0.036 3.9 x 10-6 0.036 0.054 7.8 x 10-6 N 3 4 0.050 0.072 1.4 x 10-5 Part D What is the rate of...
Rate Laws (Section)Consider the reaction of peroxydisulfate ion (S2O8 2-) with iodide ion (I - )...
Rate Laws (Section)Consider the reaction of peroxydisulfate ion (S2O8 2-) with iodide ion (I - ) in aqueous solution:S2O82 - (aq) + 3 I - (aq)→2 SO42 - (aq) + I3- (aq)At a particular temperature the initial rate of disappearance of S2O8 2 - varies with reactant concentrations in the following manner:Experiment[S2O82‑] (M)[I_] (M)Initial Rate (M/S)10.0180.0362.6 × 10-620.0270.0363.9 × 10-630.0360.0547.8 × 10-640.0500.0721.4 × 10-5(a) Determine the rate law for the reaction and state the units of the rate constant. (b)...
3. This reaction can be used to analyze for iodide ion. 10 g + 5 +...
3. This reaction can be used to analyze for iodide ion. 10 g + 5 + 6H ) ------→ 313 + 3H2O) When the rate of this reaction was studied at 25 °C, the results in the table were obtained. a. Use these data to determine the order of the reaction with respect to each of these species. Outline your reasoning in each case. [T], M [10, ), M [H],M Reaction rate, mol/L's 0.010 0.10 0.010 0.60 0.040 0.10 0.010...
The reaction between ethyl iodide and hydroxide ion in ethanol (C2H5OH) solution, C2H5I(alc) + OH(alc)+C2H5OH() +...
The reaction between ethyl iodide and hydroxide ion in ethanol (C2H5OH) solution, C2H5I(alc) + OH(alc)+C2H5OH() + (alc), has an activation energy of 86.8 kJ/mol and a frequency factor of 2.10 x 1011 M-15-7 Part A Predict the rate constant for the reaction at 31 °C 190 AED k Submit Request Answer Part B A solution of KOH in ethanol is made up by dissolving 0.304 g KOH in ethanol to form 246.0 mL of solution. Similarly, 1.586 g of C,...
11.4 The hypochlorite ion oxidizes the iodide ion in aqueous solution as represented by the equation, oci" + Iº +01+ Cl". The rate of formation of or is given by the rate law Rate = k (1"[oci") (OH) The overall reaction order is a. o b. 1 o 2 d. 3 e. 4
1. The hydroxide ion (OH-) catalyzes the reaction below, and rate data was obtained: OCI + ----> OI + Cl Experiment # [OCI]. (M) [1]. (M) [OH-]. Initial Rate (M/s) (M) 0.0040 0.0020 1.00 0.00184 2 0.0020 0.0040 1.00 0.00092 0.0020 0.0020 1.00 0.00046 0.0020 0.50 0.00046 0.0020 0.0020 0.25 0.00046 0.0020 Determine the rate law expression for this reaction (10 pts) What is the value of k (with proper units)? (5 pts)
Questions 1-5
For #1 - #5 questions of Exp. 16, complete the following chemical reaction equations (1 point each). For example, Ag+ (aq) + Cl - (aq) + AgCl (s, I white) 1. For another example, silver precipitation, AgCl (s), reacts with 15 M ammonia aqueous solution. Complete this chemical reaction equation. AgCl (s) + 2NH3 (aq) → Ag(NH3)2 + (aq) + Cl(aq) 2. The silver complex ion, one of the products from above chemical reaction equation, reacts with 6...
Consider the reaction of peroxydisulfate ion (S20;-) with iodide ion (I) in aqueous solution: S2O3- (aq) + 31- (aq) +250- (aq) +15 (aq). At a particular temperature the rate of disappearance of S20% varies with reactant concentrations in the following manner: 1 Experiment S20%- (M) I- (M) Initial Rate (M/s) 0.018 0.036 2.6 x 10-6 0.027 0.036 3.9 x 10-6 0.036 0.054 7.8 x 10-6 N 3 4 0.050 0.072 1.4 x 10-5 Part D What is the rate of...
3. This reaction can be used to analyze for iodide ion. 10 g + 5 + 6H ) ------→ 313 + 3H2O) When the rate of this reaction was studied at 25 °C, the results in the table were obtained. a. Use these data to determine the order of the reaction with respect to each of these species. Outline your reasoning in each case. [T], M [10, ), M [H],M Reaction rate, mol/L's 0.010 0.10 0.010 0.60 0.040 0.10 0.010...
The reaction between ethyl iodide and hydroxide ion in ethanol (C2H5OH) solution, C2H5I(alc) + OH(alc)+C2H5OH() + (alc), has an activation energy of 86.8 kJ/mol and a frequency factor of 2.10 x 1011 M-15-7 Part A Predict the rate constant for the reaction at 31 °C 190 AED k Submit Request Answer Part B A solution of KOH in ethanol is made up by dissolving 0.304 g KOH in ethanol to form 246.0 mL of solution. Similarly, 1.586 g of C,...
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